Consider the following electron configurations to answer the questions that follow: (i) 1s2 2s2 2p6 3s1
(ii) 1s2 2s2 2p6 3s2
(iii) 1s2 2s2 2p6 3s2 3p1
(iv) 1s2 2s2 2p6 3s2 3p4
(v) 1s2 2s2 2p6 3s2 3p5

The electron configuration that belongs to the atom with the lowest first ionization energy is .

Group of answer choices

(iv)

(i)

(iii)

(v)

(ii)

i'm not sure

explanation:

i'll try whatever you got

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.